Final answer:
The limiting reactant is 1.2 moles of O₂, which will produce 2.4 moles of H₂O according to the balanced equation 2H₂ + O₂ → 2H₂O.
Step-by-step explanation:
The question requires an understanding of stoichiometry, which involves using balanced chemical equations to determine the amounts of reactants and products involved in a chemical reaction. According to the balanced equation 2H₂ + O₂ → 2H₂O, two moles of hydrogen gas react with one mole of oxygen gas to produce two moles of water vapor. Since hydrogen and oxygen react in a 2:1 mole ratio, the limiting reactant must be identified to determine the maximum amount of water that can be produced.
Given that we have 6.9 moles of H₂ and 1.2 moles of O₂, we can calculate the moles of water produced. First, we determine the limiting reactant:
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- The reaction requires hydrogen to oxygen in a 2:1 ratio. So for 1.2 moles of O₂, we would need 2 x 1.2 = 2.4 moles of H₂.
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- We have 6.9 moles of H₂, which is more than enough to react with 1.2 moles of O₂. Therefore, oxygen is the limiting reactant.
Since 1 mole of O₂ produces 2 moles of H₂O, then 1.2 moles of O₂ will produce 1.2 x 2 = 2.4 moles of H₂O.